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Bertram Bins IV

Feb 20, 2025

is BrCl5 polar, need help?

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Zetta Hackett

Feb 20, 2025

BrCl5 has octahedral geometry with square pyramidal shape. BrCl5 has 6 effective pairs around the central Br atom, 5 of which are Br-Cl bonds, while 1 is a lone pair. Since all 6 aren't the same and because the bond dipoles don't all cancel each other out, BrCl5 must be polar.... Show More
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Zetta Hackett

Feb 20, 2025

For the best answers, search on this site https://shorturl.im/av1WdTo determine the most polar molecule, you first look at the shape of the molecule. CF4 would be a tetrahedral molecule because Carbon has no pairs of lone electrons. BrCl5 would be a trigonal bipyramid because Bromine has no pairs of lone electrons. PCl5 would be a trigonal bipyramid because Phosphorous has no pairs of lone electrons. SCl6 would be a square bipyramid because Sulfur has no pairs of lone electrons. XeF2 would be a linear molecule with lone pairs of electrons on either side of Xenon. Because none of these are polar based on the shape, we now look at the size of the molecules. London Dispersion Forces are the strongest in the largest molecules. LD forces can determine polarity. I would have to say that the largest molecule of this group is BrCl5. ANSWER: BrCl5... Show More
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Zetta Hackett

Feb 20, 2025

the diffrence in electronegativities of Cl and Br is 3.0-2.8=0.2 so it is a non-polar molecule... Show More
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